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16.10: Titration of a Polyprotic Acid

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Chemistry

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Titration of a Polyprotic Acid
 
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16.10: Titration of a Polyprotic Acid

A polyprotic acid contains more than one ionizable hydrogen and undergoes a stepwise ionization process.  If the acid dissociation constants of the ionizable protons differ sufficiently from each other, then the titration curve for such polyprotic acid generates a distinct equivalence point for each of its ionizable hydrogens. Therefore, titration of a diprotic acid results in the formation of two equivalence points, whereas the titration of a triprotic acid results in the formation of three equivalence points on the titration curve.

Carbonic acid, H2CO3, is an example of a weak diprotic acid. The first ionization of carbonic acid yields hydronium ions and bicarbonate ions in small amounts.

First ionization:

Eq1

The bicarbonate ion can also act as an acid. It ionizes and forms hydronium ions and carbonate ions in even smaller quantities.

Second ionization:

Eq2

The Ka1 is larger than the Ka2 by a factor of 104. Therefore, when H2CO3 is titrated with a strong base like NaOH, it produces two distinct equivalence points for each ionizable hydrogen.

Phosphoric acid, a triprotic acid, ionizes in three steps:

First ionization:

Eq3

Second ionization:

Eq4

Third ionization:

Eq5

When H3PO4 is titrated with a strong base like KOH, it produces three equivalence points for each ionizable hydrogen. However, as HPO42− is a very weak acid, the third equivalence point is not easily discernible on the titration curve.

This text is adapted from Openstax, Chemistry 2e, Section 14.5: Polyprotic Acids.

Tags

Polyprotic Acid Ionizable Protons Ka Dissociation Constant Sulfurous Acid Titration Curve Strong Base Sodium Hydroxide Hydrogen Sulfite Ions Equivalence Point PH Half-equivalence Point Second Ionizable Proton Diprotic Acid Neutralization Step Triprotic Phosphoric Acid

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